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18 Dec 2019
A calorimeter contains 18.0 mL of water at 15.0 degrees Celcius . When 1.80 g of X (a substance with a molar mass of 42.0 g/mol) is added, it dissolves via the reaction X(s)+H2O(l)-->X(aq) and the temperature of the solution increases to 30.0 degrees Celcius . Calculate the enthalpy change, for this reaction per mole of X.Assume that the specific heat and density of the resulting solution are equal to those of water [4.18 J/g C and 1.00 g/mL ] and that no heat is lost to the calorimeter itself, nor to the surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures.
A calorimeter contains 18.0 mL of water at 15.0 degrees Celcius . When 1.80 g of X (a substance with a molar mass of 42.0 g/mol) is added, it dissolves via the reaction X(s)+H2O(l)-->X(aq) and the temperature of the solution increases to 30.0 degrees Celcius . Calculate the enthalpy change, for this reaction per mole of X.Assume that the specific heat and density of the resulting solution are equal to those of water [4.18 J/g C and 1.00 g/mL ] and that no heat is lost to the calorimeter itself, nor to the surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures.
Keith LeannonLv2
31 Dec 2019